Skip to main content
Ch.10 - Gases: Their Properties & Behavior
McMurry - Chemistry 8th Edition
McMurry8th EditionChemistryISBN: 9781292336145당신이 사용하는 게 아니라요?교과서 변경
모든 교과서McMurry 8th EditionCh.10 - Gases: Their Properties & Behavior문제 89b
10장, 문제 89b

Chlorine gas was first prepared in 1774 by the oxidation of NaCl with MnO2: 2 NaCl(s) + 2 H2SO4(l) + MnO2(s) → Na2SO4(s) + MnSO4(s) + 2 H2O(g) + Cl2(g) Assume that the gas produced is saturated with water vapor at a partial pressure of 28.7 mm Hg and that it has a volume of 0.597 L at 27 °C and 755 mm Hg pressure. (b) How many grams of NaCl were used in the experiment, assuming complete reaction?

검증된 단계별 안내
1
Identify the relevant chemical reaction: \(2 \text{NaCl} + 2 \text{H}_2\text{SO}_4 + \text{MnO}_2 \rightarrow \text{Na}_2\text{SO}_4 + \text{MnSO}_4 + 2 \text{H}_2\text{O} + \text{Cl}_2\).
Use the ideal gas law \(PV = nRT\) to find the moles of \(\text{Cl}_2\) gas produced. Remember to adjust the pressure to account for water vapor: \(P_{\text{dry}} = 755 \text{ mm Hg} - 28.7 \text{ mm Hg}\).
Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature.
Calculate the moles of \(\text{Cl}_2\) using the ideal gas law with the adjusted pressure, volume, and temperature.
Use stoichiometry to convert moles of \(\text{Cl}_2\) to moles of \(\text{NaCl}\), and then convert moles of \(\text{NaCl}\) to grams using its molar mass.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
5m

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the amount of substances consumed and produced in a reaction. In this case, understanding the stoichiometric relationships between NaCl and Cl2 is essential to calculate the mass of NaCl used.
추천 영상:
가이드 코스
01:16
Stoichiometry Concept

Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is crucial for determining the number of moles of Cl2 produced in the reaction, as it allows us to convert the measured volume and pressure of the gas into moles, which can then be related back to the mass of NaCl.
추천 영상:
가이드 코스
01:15
Ideal Gas Law Formula

Partial Pressure

Partial pressure is the pressure exerted by a single component of a mixture of gases. In this scenario, the total pressure of the gas mixture includes the partial pressure of Cl2 and the water vapor. To find the pressure of Cl2 alone, we must subtract the partial pressure of water vapor from the total pressure, which is necessary for accurate calculations using the Ideal Gas Law.
추천 영상:
가이드 코스
00:48
Partial Pressure Calculation
관련 실천
교과서 질문

Natural gas is a mixture of hydrocarbons, primarily methane 1CH42 and ethane 1C2H62. A typical mixture might have Xmethane = 0.915 and Xethane = 0.085. Let's assume that we have a 15.50 g sample of natural gas in a volume of 15.00 L at a temperature of 20.00 °C. (a) How many total moles of gas are in the sample?

464
views
교과서 질문
A 20.0-L flask contains 0.776 g of He and 3.61 g of CO2 at 300 K. (a) What is the partial pressure of He in mm Hg?
632
views
교과서 질문

Natural gas is a mixture of hydrocarbons, primarily methane (CH4) and ethane (C2H6). A typical mixture might have Xmethane = 0.915 and Xethane = 0.085. Let's assume that we have a 15.50 g sample of natural gas in a volume of 15.00 L at a temperature of 20.00 °C. (c) What is the partial pressure of each component in the sample in atmospheres?

541
views
교과서 질문

Natural gas is a mixture of hydrocarbons, primarily methane (CH4) and ethane (C2H6). A typical mixture might have Xmethane = 0.915 and Xethane = 0.085. Let's assume that we have a 15.50 g sample of natural gas in a volume of 15.00 L at a temperature of 20.00 °C. (b) What is the pressure of the sample in atmospheres?

1359
views
교과서 질문

Chlorine gas was first prepared in 1774 by the oxidation of NaCl with MnO2: 2 NaCl(s) + 2 H2SO4(l) + MnO2(s) → Na2SO4(s) + MnSO4(s) + 2 H2O(g) + Cl2(g) Assume that the gas produced is saturated with water vapor at a partial pressure of 28.7 mm Hg and that it has a volume of 0.597 L at 27 °C and 755 mm Hg pressure. (a) What is the mole fraction of Cl2 in the gas?

380
views
교과서 질문
A sample of magnesium metal reacts with aqueous HCl to yield H2 gas: Mg1s2 + 2 HCl1aq2¡MgCl21aq2 + H21g2 The gas that forms is found to have a volume of 3.557 L at 25 °C and a pressure of 747 mm Hg. Assuming that the gas is saturated with water vapor at a partial pressure of 23.8 mm Hg, what is the partial pressure in millimeters of mercury of the H2? How many grams of magnesium metal were used in the reaction?
1183
views